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INNOVATIVE LESSON PLAN

INNOVATIVE LESSON PLAN. PRASANTH M ST JACOB’S TRAINING COLLEGE. Lewis acid. Lewis base. Complex ion. Lewis acid. Lewis base. Complex ion. Coordination Chemistry. Transition metals act as Lewis acids Form complexes/complex ions Fe 3+ (aq) + 6CN - (aq)  [Fe(CN) 6 ] 3- (aq)

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INNOVATIVE LESSON PLAN

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  1. INNOVATIVE LESSON PLAN PRASANTH M ST JACOB’S TRAINING COLLEGE

  2. Lewis acid Lewis base Complex ion Lewis acid Lewis base Complex ion Coordination Chemistry • Transition metals act as Lewis acids • Form complexes/complex ions Fe3+(aq) + 6CN-(aq)  [Fe(CN)6]3-(aq) Ni2+(aq) + 6NH3(aq)  [Ni(NH3)6]2+(aq) Complex with a net charge = complex ion Complexes have distinct properties

  3. Coordination Chemistry • Coordination compound • Compound that contains 1 or more complexes • Example • [Co(NH3)6]Cl3 • [Cu(NH3)4][PtCl4] • [Pt(NH3)2Cl2]

  4. Coordination Chemistry • Coordination sphere • Metal and ligands bound to it • Coordination number • number of donor atoms bonded to the central metal atom or ion in the complex • Most common = 4, 6 • Determined by ligands • Larger ligands and those that transfer substantial negative charge to metal favor lower coordination numbers

  5. Coordination Chemistry Complex charge = sum of charges on the metal and the ligands [Fe(CN)6]3-

  6. Coordination Chemistry Complex charge = sum of charges on the metal and the ligands [Fe(CN)6]3- +3 6(-1)

  7. Coordination Chemistry Neutral charge of coordination compound = sum of charges on metal, ligands, and counterbalancing ions [Co(NH3)6]Cl2 neutral compound

  8. Coordination Chemistry Neutral charge of coordination compound = sum of charges on metal, ligands, and counterbalancing ions [Co(NH3)6]Cl2 +2 6(0) 2(-1)

  9. Coordination Chemistry • Ligands • classified according to the number of donor atoms • Examples • monodentate = 1 • bidentate = 2 • tetradentate = 4 • hexadentate = 6 • polydentate = 2 or more donor atoms

  10. Coordination Chemistry • Ligands • classified according to the number of donor atoms • Examples • monodentate = 1 • bidentate = 2 • tetradentate = 4 • hexadentate = 6 • polydentate = 2 or more donor atoms chelating agents

  11. Ligands • Monodentate • Examples: • H2O, CN-, NH3, NO2-, SCN-, OH-, X- (halides), CO, O2- • Example Complexes • [Co(NH3)6]3+ • [Fe(SCN)6]3-

  12. Ligands • Bidentate • Examples • oxalate ion = C2O42- • ethylenediamine (en) = NH2CH2CH2NH2 • ortho-phenanthroline (o-phen) • Example Complexes • [Co(en)3]3+ • [Cr(C2O4)3]3- • [Fe(NH3)4(o-phen)]3+

  13. Ligands oxalate ion ethylenediamine * * * * ortho-phenanthroline * * Donor Atoms

  14. Ligands oxalate ion ethylenediamine H C C O M N M

  15. Ligands

  16. Ligands • Hexadentate • ethylenediaminetetraacetate (EDTA) = (O2CCH2)2N(CH2)2N(CH2CO2)24- • Example Complexes • [Fe(EDTA)]-1 • [Co(EDTA)]-1

  17. Ligands EDTA * * * * * * Donor Atoms

  18. Ligands EDTA O H C N M

  19. Ligands EDTA

  20. Common Geometries of Complexes Coordination Number Geometry 2 Linear

  21. Common Geometries of Complexes Coordination Number Geometry 2 Linear Example: [Ag(NH3)2]+

  22. Common Geometries of Complexes Coordination Number Geometry 4 tetrahedral (most common) square planar (characteristic of metal ions with 8 d e-’s)

  23. Common Geometries of Complexes Coordination Number Geometry 4 tetrahedral Examples: [Zn(NH3)4]2+, [FeCl4]- square planar Example: [Ni(CN)4]2-

  24. Common Geometries of Complexes Coordination Number Geometry 6 octahedral

  25. Common Geometries of Complexes Coordination Number Geometry 6 Examples: [Co(CN)6]3-, [Fe(en)3]3+ octahedral

  26. Porphine, an important chelating agent found in nature

  27. Metalloporphyrin

  28. Myoglobin, a protein that stores O2 in cells

  29. Coordination Environment of Fe2+ in Oxymyoglobin and Oxyhemoglobin

  30. Coordination Environment of Fe2+ in Oxymyoglobin and Oxyhemoglobin

  31. Arterial Blood Strong field large  Bright red due to absorption of greenish light

  32. Venous Blood Weak field small  Bluish color due to absorption of orangish light

  33. End of Presentation

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